Homework Help: AP Chemistry

Posted by Sally Perez on Monday, March 8, 2010 at 9:02pm.

Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of a monoprotic strong acid HX. (a) How many moles of HX have been added at the equivalence point? (b) What is the predominant form of B at the equivalence point? (c) What factor determines the pH at the equivalence point? (d) Which indicator, phenolphthalein or methyl red, is likely to be the better choice for this titration?

AP Chemistry - DrBob222, Monday, March 8, 2010 at 9:11pm
a. moles HX added = M x L.
b. B + HX ==> BH^+ + X^-
c. The hydrolysis of the salt BH^+. Said another way, the strength of BH^+ as an acid.
d. Phenolphthalein changes color at pH about 9. Methyl red changes color about 5. Which do you think?
AP Chemistry - serjon, Wednesday, March 17, 2010 at 12:53pm
a. 2.7 x 10 -3 moles or 0.0027
b. BH + (aq)
c. Already given.
d. phenolphthalein
AP Chemistry - Anonymous, Tuesday, September 21, 2010 at 12:35am
hi
AP Chemistry - Diggity dogg, Wednesday, March 16, 2011 at 10:13pm
hi to you. is this right?
AP Chemistry - Boxer Boy, Wednesday, December 7, 2011 at 7:58pm
c. is actually methyl red
AP Chemistry - Allison, Sunday, March 4, 2012 at 1:47pm
For c it is both the Ka for BH^+ and concentration of BH^+ to determine pH at the equivalence point.

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